The balloon of air inflated which does 475kj of work to the air in the balloon. the balloon then received 35kj of energy from the surrounding air. How much internal energy did the gas inside the balloon gain or lose?
To determine the change in internal energy of the gas inside the balloon, we need to consider the work done on the gas and the energy transferred to it.
Given:
Work done on the gas = 475 kJ
Energy transferred to the gas = 35 kJ
The change in internal energy (ΔU) can be calculated using the first law of thermodynamics, which states that the change in internal energy of a system is equal to the sum of the heat added to the system and the work done on the system:
ΔU = Q + W
Where:
ΔU = change in internal energy
Q = heat added to the system
W = work done on the system
In this case, the work is done on the gas, so W is positive (+475 kJ). The energy transferred to the gas from the surrounding air is heat, so Q is positive (+35 kJ).
Substituting the given values into the equation:
ΔU = 35 kJ + 475 kJ
ΔU = 510 kJ
Therefore, the gas inside the balloon gained 510 kJ of internal energy.
To determine the change in internal energy of the gas inside the balloon, we need to consider the work done on the gas and the energy transferred to or from the gas. The change in internal energy (ΔU) can be calculated using the first law of thermodynamics:
ΔU = Q - W
Where:
ΔU = Change in internal energy
Q = Heat transferred to or from the gas
W = Work done on the gas
In this case, the work done on the gas is positive (475 kJ) as the air inside the balloon is being inflated. The energy transferred to the gas is also positive (35 kJ) as it is receiving energy from the surrounding air.
Thus, plugging in the values into the equation:
ΔU = Q - W
ΔU = 35 kJ - 475 kJ
ΔU = -440 kJ
Therefore, the gas inside the balloon has lost 440 kJ of internal energy.
To determine the change in internal energy of the gas inside the balloon, we need to consider the work done on the gas and the energy transferred to the gas.
Given:
Work done on the gas (W) = 475 kJ
Energy transferred to the gas (Q) = 35 kJ
According to the first law of thermodynamics, the change in internal energy (ΔU) of a system is given by the equation:
ΔU = Q - W
Substituting the given values, we have:
ΔU = 35 kJ - 475 kJ
Calculating the change in internal energy:
ΔU = -440 kJ
Therefore, the gas inside the balloon experienced a decrease in internal energy of 440 kJ.